When octane, C3H18, undergoes combustion the following reaction occurs: --C8 H8 + -O2 → _CO2 + -__H2O When 2.15 g of Cg Hg is combusted in a bomb calorimeter, the temperature of the calorimeter and 700 mL of liquid water increases from 25.00°C to 34.6°C. In a separate experiment, the heat capacity of the calorimeter is measured to be 7.794 kJ/°C. What is the heat of reaction for the combustion of a mole of C3H18? (Specific heat capacity of liquid water = 4.184 J/g.°C)

When octane, C3H18, undergoes combustion the following reaction occurs: --C8 H8 + -O2 → _CO2 + -__H2O When 2.15 g of Cg Hg is combusted in a bomb calorimeter, the temperature of the calorimeter and 700 mL of liquid water increases from 25.00°C to 34.6°C. In a separate experiment, the heat capacity of the calorimeter is measured to be 7.794 kJ/°C. What is the heat of reaction for the combustion of a mole of C3H18? (Specific heat capacity of liquid water = 4.184 J/g.°C)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + 0,(g) → CO,(g) + 2 H,O(1) ΔΗ --764 kJ How much methanol, in grams, must be burned to produce 837 kJ of heat?
Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request Answer
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
Fructose, C6H12O6(s), is a sugar closely related to glucose. A 0.755 g sample of fructose was combusted with excess oxygen in a bomb calorimeter, containing 500.0 g of water. The heat capacity of the empty calorimeter was 208 J/K. The temperature of the calorimeter and the water rose from 22.00°C to 27.12°C due to the combustion reaction, which formed CO₂(g) and liquid water. What is the energy change, AU (in kJ), for the combustion of one mole of fructose under these conditions? O +254 O-15600 -2810 +520 -804
The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid.In a particular bomb calorimeter (initially at room temperature), the combustion of 0.2745 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.85 °C.When a 0.2999-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.59 °C.What is the energy of combustion per unit mass of the unknown substance?
A 1.615-g sample of benzoic acid, C7H6O2 (122.12 g/mol) was burned in a bomb calorimeter with excessoxygen. The temperature of the calorimeter and the water before combustion was 17.49 °C; after combustionthe calorimeter and the water had a temperature of 27.28 °C. The calorimeter had a heat capacity of 832 J/K,and contained 0.837 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of benzoicacid.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1400. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (CH-CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 21.00 °C to 42.00 °C over a time of 8.5 minutes. Next, 5.190 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 21.00 °C to 63.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. exothermic C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(g) Be…
Fructose, C6H12O6(s), is a sugar closely related to glucose.. A 0.755 g sample of fructose was combusted with excess oxygen in a bomb calorimeter, containing 500.0 g of water. The heat capacity of the empty calorimeter was 208 J/K. The temperature of the calorimeter and the water rose from 22.00°C to 27.12°C due to the combustion reaction, which formed CO2(g) and liquid water. What is the energy change, AU (in kJ), for the combustion of one mole of fructose under these conditions? -15600 -2810 +520 +254 -804
The combustion of toluene has a AErxn of -3.91 x 10³ kJ/mol. When 1.30 g of toluene (C7H8) undergoes combustion in a bomb calorimeter, the temperature rises from 22.80 °C to 36.11 °C. Find the heat capacity of the bomb calorimeter. Express your answer using three significant figures. Ccal = 17| ΑΣΦ ? kJ/°C
A student has a coffee-cup calorimeter with 50.0 g of water at 21.5oC. They introduce 15.525 g of magnesium metal initially at 100.0oC. The final temperature of the calorimeter came to 27.2oC. What is Cmagnesium in J/g-K?
2) The combustion of 0.25 g sucrose, C1HO11, in a bomb calorimeter causes the temperature to rise from 24.9 to 28.3 °C. If the heat capacity of the calorimeter is 4.90 kJ/°C, calculate the heat of combustion of sucrose in kJ/g.
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.461-g sample of 2-naphthylacetic acid (C12H1002) in a bomb calorimeter containing 1150. g water. The temperature increases from 24.70 °C to 27.20 °C. The specific heat capacity of water is 4.184 J g1 oC-1. The combustion enthalpy is -5779 kJ/mol 2-naphthylacetic acid. C12H1002(s) + 27/2 02(g) –→12 CO2(g) + 5 H20(1) A,H° -5779 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter= orc J/C